www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1.

chem10b 15.2-13 The equilibrium expression for Kp for the reaction below is __________. 2O3 (g)

3O2 (g)

Student Response

Correct Answer

A. B. C. D. E.

2.

chem10b 15.2-18 The Keq for the equilibrium below is 0.112 at 700 °C.

SO2 (g) + O2 (g) SO3 (g) What is the value of Keq at this temperature for the following reaction?

SO3 (g)

SO2 (g) +

Student Response A. 0.224 B. 0.112

O2 (g)

Correct Answer

C. 0.0125 D. 8.93 E. -0.112

3.

chem10b 15.2-12 Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N2O4 (g) = 2NO2 (g)

Student Response

Correct Answer

A. [NO2]2[N2O4] B. [NO2][N2O4] C. D. [NO2]2/[N2O4] E.

4.

chem10b 15.5-3 The Kp for the reaction below is 1.49 × 108 at 100 °C: CO (g) + Cl2 (g) → COCl2 (g) In an equilibrium mixture of the three gases, PCO = PCl2 = 8.60 × 10-4 atm. The partial pressure of the product, phosgene (COCl2), is __________ atm.

Student Response A. 2.01 × 1014 B. 1.28 × 105 C. 1.10 × 102 D. 1.72 × 1011 E. 4.96 × 10-15

5.

chem10b 15.2-19

Correct Answer

The Keq for the equilibrium below is 0.112 at 700 °C. SO2 (g) ½ O2 (g) + SO3 (g) What is the value of Keq at this temperature for the following reaction? 2SO3 (g) 2SO2 (g) + O2 (g)

Student Response

Correct Answer

A. 2.99 B. 4.46 C. 79.7 D. 8.93 E. 17.86

6.

chem10b 15.2-20 At 1000 K, the equilibrium constant for the reaction 2NO (g) + Br2 (g)

2NOBr (g)

is Kp = 0.013. Calculate Kp for the reverse reaction, 2NOBr (g)

2NO (g) + Br2 (g).

Student Response

Correct Answer

A. 1.6 × 10-4 B. 1.1 C. 77 D. 0.99 E. 0.013

7.

chem10b 15.2-38 The effect of a catalyst on an equilibrium is to __________.

Student Response

Correct Answer

A. increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture B. increase the equilibrium constant so that products are favored C. increase the rate of the forward reaction only D. slow the reverse reaction only E. shift the equilibrium to the right Score: 8.

1/1

chem10b 15.2-29 The reaction below is exothermic: 2SO2 (g) + O2 (g)

2SO3 (g)

Le Ch telier's Principle predicts that __________ will result in an increase in the number of moles of SO3 (g) in the reaction container.

Student Response

Correct Answer

A. removing some oxygen B. decreasing the pressure C. increasing the temperature D. increasing the pressure E. increasing the volume of the container

9.

chem10b 15.2-21 Consider the following equilibrium. 2 SO2 (g) + O2 (g)

2 SO3 (g)

The equilibrium cannot be established when __________ is/are placed in a 1.0-L container.

Student Response A. 0.25 mol of SO2 (g) and 0.25 mol of SO3 (g) B. 0.50 mol O2 (g) and 0.50 mol SO3 (g) C. 1.0 mol SO3 (g)

Correct Answer

D. 0.25 mol SO2 (g) and 0.25 mol O2 (g) E. 0.75 mol SO2 (g)

10. chem10b 15.2-28 Of the following equilibria, only __________ will shift to the left in response to a decrease in volume.

Student Response A. H2 (g) + Cl2 (g)

2 HCl (g)

B. 4 Fe (s) + 3 O2 (g) C. N2 (g) + 3 H2 (g) D. 2 SO3 (g) E. 2HI (g)

Correct Answer

2 Fe2O3 (s) 2 NH3 (g)

2 SO2 (g) + O2 (g) H2 (g) + I2 (g)

11. chem10b 15.1-12 A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g)

2IBr (g)

When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is __________.

Student Response A. 2.8 B. 110 C. 4.0 D. 6.1 E. 11 Score:

1/1

12. chem10b 15.2-17 The Keq for the equilibrium below is 0.112 at 700 °C.

Correct Answer

SO2 (g) + O2 (g) SO3 (g) What is the value of Keq at this temperature for the following reaction? 2SO2 (g) + O2 (g)

2SO3 (g)

Student Response

Correct Answer

A. 0.0125 B. 0.0560 C. 0.335 D. 0.112 E. 0.224

1.

chem10b 15.2-2 What role did Karl Bosch play in development of the Haber-Bosch process?

Student Response

Correct Answer

A. He discovered the reaction conditions necessary for formation of ammonia. B. He was the German industrialist who financed the research done by Haber. C. Haber was working in his lab with his instructor at the time he worked out the process. D. He originally isolated ammonia from camel dung and found a method for purifying it. E. He developed the equipment necessary for industrial production of ammonia.

2.

chem10b 15.5-5 The equilibrium constant (Kp) for the reaction below is 7.00 × 10-2 at 22 °C: NH4HS (s) → NH3 (g) + H2S (g) A sample of NH4HS is placed in an evacuated container and allowed to come to equilibrium. The partial pressure of NH3 is then increased by the addition of 0.590 atm of NH3. The partial

pressure of H2S at equilibrium is now __________ atm.

Student Response

Correct Answer

A. 0.855 B. 0.101 C. 0.691 D. 0.119 E. 0.265 Score: 3.

1/1

chem10b 15.2-27 Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)

2NO (g) + Br2 (g)

A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained .46 mol of NOBr. How many moles of NO and Br2, respectively, are in the flask at equilibrium?

Student Response

Correct Answer

A. 0.46, 0.46 B. 0.18, 0.18 C. 0.18, 0.090 D. 0.18, 0.360 E. 0.46, 0.23

4.

chem10b 15.2-11 The value of Keq for the following reaction is 0.25: SO2 (g) + NO2 (g)

SO3 (g) + NO (g)

The value of Keq at the same temperature for the reaction below is __________. 2SO2 (g) + 2NO2 (g)

Student Response

2SO3 (g) + 2NO (g)

Correct Answer

A. 0.062 B. 0.50 C. 0.25 D. 0.12 E. 16

5.

chem10b 15.2-28 Of the following equilibria, only __________ will shift to the left in response to a decrease in volume.

Student Response A. 2 SO3 (g) B. 2HI (g)

Correct Answer

2 SO2 (g) + O2 (g) H2 (g) + I2 (g)

C. N2 (g) + 3 H2 (g) D. H2 (g) + Cl2 (g)

2 NH3 (g) 2 HCl (g)

E. 4 Fe (s) + 3 O2 (g)

6.

2 Fe2O3 (s)

chem10b 15.1-5 A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g)

H2(g) + I2(g)

When the system comes to equilibrium at 425 °C, PHI = 0.708 atm, and

PH2 = PI2

The value of Kp at this temperature is __________.

Student Response A. 54.3 B. 1.30 × 10-2 C. Kp cannot be calculated for this gas reaction when the volume of the reaction vessel is not given. D. 6.80 × 10-2

Correct Answer

E. 1.84 × 10-2

7.

chem10b 15.1-8 Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) < -- > 2NO2 (g) A 1.00-L flask is charged with 0.0400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is __________.

Student Response

Correct Answer

A. 2.2 × 10-4 B. 0.022 C. 0.22 D. 0.87 E. 13

8.

chem10b 15.2-18 The Keq for the equilibrium below is 0.112 at 700 °C.

SO2 (g) + O2 (g) SO3 (g) What is the value of Keq at this temperature for the following reaction?

SO3 (g)

SO2 (g) +

Student Response A. 0.224 B. 0.112 C. 8.93 D. -0.112 E. 0.0125

O2 (g)

Correct Answer

9.

chem10b 15.2-5 Which one of the following will change the value of an equilibrium constant?

Student Response

Correct Answer

A. varying the initial concentrations of reactants B. changing temperature C. adding other substances that do not react with any of the species involved in the equilibrium D. varying the initial concentrations of products E. changing the volume of the reaction vessel

10. chem10b 15.2-33 Consider the following reaction at equilibrium: 2NH3 (g)

N2 (g) + 3H2 (g)

Le Ch telier's principle predicts that the moles of H2 in the reaction container will increase with __________

Student Response

Correct Answer

A. an increase in total pressure by the addition of helium gas (V and T constant) B. a decrease in the total pressure (T constant) C. some removal of NH3 from the reaction vessel (V and T constant) D. addition of some N2 to the reaction vessel (V and T constant) E. a decrease in the total volume of the reaction vessel (T constant) Score:

1/1

11. chem10b 15.2-38 The effect of a catalyst on an equilibrium is to __________.

Student Response A. slow the reverse reaction only

Correct Answer

B. increase the equilibrium constant so that products are favored C. increase the rate of the forward reaction only D. shift the equilibrium to the right E. increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture

12. chem10b 15.2-34 Consider the following reaction at equilibrium: 2CO2 (g)

2CO (g) + O2 (g) ΔH° = -514 kJ

Le Ch telier's principle predicts that adding O2 (g) to the reaction container will _________.

Student Response

Correct Answer

A. decrease the partial pressure of CO2 (g) at equilibrium B. increase the value of the equilibrium constant C. increase the partial pressure of CO2 (g) at equilibrium D. increase the partial pressure of CO (g) at equilibrium E. decrease the value of the equilibrium constant

1.

chem10b 15.2-27 Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)

2NO (g) + Br2 (g)

A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained are in the flask at equilibrium?

of NOBr. How many moles of NO and Br2, respectively,

Student Response

Correct Answer

A. 0.46, 0.46 B. 0.18, 0.18 C. 0.18, 0.090 D. 0.18, 0.360 E. 0.46, 0.23

2.

chem10b 15.1-12 A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g)

2IBr (g)

When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is __________.

Student Response

Correct Answer

A. 2.8 B. 6.1 C. 11 D. 4.0 E. 110

3.

chem10b 15.2-9 The equilibrium constant for the gas phase reaction 2NH3 (g)

N2 (g) + 3H2 (g)

is Keq = 230 at 300 °C. At equilibrium, __________.

Student Response A. reactants predominate B. only reactants are present C. roughly equal amounts of products and reactants are present

Correct Answer

D. only products are present E. products predominate

4.

chem10b 15.2-15 The Keq for the equilibrium below is 7.52 × 10-2 at 480 °C. 2Cl2 (g) + 2H2O (g)

4HCl (g) + O2 (g)

What is the value of Keq at this temperature for the following reaction? 4HCl (g) + O2 (g)

2Cl2 (g) + 2H2O (g)

Student Response

Correct Answer

A. 13.3 B. 0.150 C. 5.66 × 10-3 D. 0.0752 E. -0.0752

5.

chem10b 15.2-14 The Keq for the equilibrium below is 7.52 × 10-2 at 480 °C. 2Cl2 (g) + 2H2O (g)

4HCl (g) + O2 (g)

What is the value of Keq at this temperature for the following reaction?

Cl2 (g) + H2O (g)

2HCl (g) +

Student Response A. 5.66 × 10-3 B. 0.274 C. 0.0752 D. 0.150 E. 0.0376

O2 (g)

Correct Answer

6.

chem10b 15.2-29 The reaction below is exothermic: 2SO2 (g) + O2 (g)

2SO3 (g)

Le Ch telier's Principle predicts that __________ will result in an increase in the number of moles of SO3 (g) in the reaction container.

Student Response

Correct Answer

A. decreasing the pressure B. increasing the pressure C. removing some oxygen D. increasing the temperature E. increasing the volume of the container

7.

chem10b 15.5-4 At 900 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 + O2 (g) → 2SO3 (g) At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is __________ atm.

Student Response

Correct Answer

A. 6.20 × 10-4 B. 4.21 × 10-3 C. 82.0 D. 40.2 E. 192 Score: 8.

1/1

chem10b 15.1-7 At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide:

H2 (g) + Br2 (g)

2HBr (g)

A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.566 mol of H2 present. At equilibrium, there are __________ mol of Br2 present in the reaction vessel.

Student Response

Correct Answer

A. 0.440 B. 0.566 C. 0.232 D. 0.324 E. 0.000 Score: 9.

1/1

chem10b 15.2-25 How does the reaction quotient of a reaction (Q) differ from the equilibrium constant (Keq) of the same reaction?

Student Response

Correct Answer

A. Q does not depend on the concentrations or partial pressures of reaction components. B. Q is the same as Keq when a reaction is at equilibrium. C. Q does not change with temperature. D. K does not depend on the concentrations or partial pressures of reaction components. E. Keq does not change with temperature, whereas Q is temperature dependent. Score:

0/1

10. chem10b 15.4-5 Le Chatelier's principle states that if a system at equilibrium is disturbed, the equilibrium will shift to minimize the disturbance.

Student Response

Value

Correct Answer

11. chem10b 15.5-5 The equilibrium constant (Kp) for the reaction below is 7.00 × 10-2 at 22 °C: NH4HS (s) → NH3 (g) + H2S (g) A sample of NH4HS is placed in an evacuated container and allowed to come to equilibrium. The partial pressure of NH3 is then increased by the addition of 0.590 atm of NH3. The partial pressure of H2S at equilibrium is now __________ atm.

Student Response

Correct Answer

A. 0.119 B. 0.691 C. 0.265 D. 0.855 E. 0.101

12. chem10b 15.2-31 In which of the following reactions would increasing pressure at constant temperature not change the concentrations of reactants and products, based on Le Ch

Student Response A. 2N2 (g) + O2 (g) B. N2 (g) + O2 (g)

1.

Correct Answer 2N2O (g)

2NO (g)

C. N2 (g) + 2O2 (g)

2NO2 (g)

D. N2 (g) + 3H2 (g)

2NH3 (g)

E. N2O4 (g)

telier's principle?

2NO2 (g)

chem10b 15.2-34 Consider the following reaction at equilibrium: 2CO2 (g)

2CO (g) + O2 (g) ΔH° = -514 kJ

Le Ch telier's principle predicts that adding O2 (g) to the reaction container will __________.

Student Response

Correct Answer

A. increase the partial pressure of CO (g) at equilibrium B. decrease the partial pressure of CO2 (g) at equilibrium C. increase the partial pressure of CO2 (g) at equilibrium D. decrease the value of the equilibrium constant E. increase the value of the equilibrium constant

2.

chem10b 15.2-36 Consider the following reaction at equilibrium. 2CO2 (g)

2CO (g) + O2 (g) ΔH° = -514 kJ

Le Ch telier's principle predicts that the equilibrium partial pressure of CO (g) can be maximized by carrying out the reaction __________.

Student Response

Correct Answer

A. at high temperature and high pressure B. at high temperature and low pressure C. at low temperature and low pressure D. at low temperature and high pressure E. in the presence of solid carbon

3.

chem10b 15.2-10 The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is __________. (1) SO2 (g) + (1/2) O2 (g) SO3 (g) (2) 2SO3 (g) 2SO2 (g) + O2 (g)

Student Response A. 1/K2

Correct Answer

B. K2 C. 1/2K D. -K2 E. 2K

4.

chem10b 15.2-8 The equilibrium constant for the gas phase reaction N2 (g) + 3H2 (g)

2NH3 (g)

is Keq = 4.34 × 10-3 at 300 °C. At equilibrium, __________.

Student Response

Correct Answer

A. products predominate B. only products are present C. reactants predominate D. roughly equal amounts of products and reactants are present E. only reactants are present

5.

chem10b 15.2-33 Consider the following reaction at equilibrium: 2NH3 (g)

N2 (g) + 3H2 (g)

Le Ch telier's principle predicts that the moles of H2 in the reaction container will increase with __________

Student Response A. an increase in total pressure by the addition of helium gas (V and T constant) B. some removal of NH3 from the reaction vessel (V and T constant) C. a decrease in the total volume of the reaction vessel (T constant)

Correct Answer

D. a decrease in the total pressure (T constant) E. addition of some N2 to the reaction vessel (V and T constant)

6.

chem10b 15.1-9 At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103. 2NO (g) < -- > N2 (g) + O2 (g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is __________ atm.

Student Response

Correct Answer

A. 294 B. 18.1 C. 6.00 D. 1.50 × 10-2 E. 35.7 Score: 7.

0/1

chem10b 15.2-23 The equilibrium-constant expression for the reaction Ti (s) + 2Cl2 (g)

TiCl4 (l)

is given by

Student Response A. B. C. [Cl2 (g)]-2 D. E.

Correct Answer

Score: 8.

1/1

chem10b 15.1-6 Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC2H3O2 (aq)

C2H3O2- (aq) + H+ (aq)

At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: and __________.

The equilibrium constant, Keq, for the ionization of acetic acid at

Student Response

is

Correct Answer

A. 1.75 × 10-7 B. 1.79 × 10-5 C. 5.71 × 104 D. 5.71 × 106 E. 0.100

9.

chem10b 15.2-21 Consider the following equilibrium. 2 SO2 (g) + O2 (g)

2 SO3 (g)

The equilibrium cannot be established when __________ is/are placed in a 1.0-L container.

Student Response

Correct Answer

A. 0.50 mol O2 (g) and 0.50 mol SO3 (g) B. 0.25 mol SO2 (g) and 0.25 mol O2 (g) C. 0.75 mol SO2 (g) D. 0.25 mol of SO2 (g) and 0.25 mol of SO3 (g) E. 1.0 mol SO3 (g)

10. chem10b 15.1-7 At elevated temperatures, molecular hydrogen and molecular bromine react to partially form

hydrogen bromide: H2 (g) + Br2 (g)

2HBr (g)

A mixture of 0.682 mol of H2 and 0.440 mol of Br2 is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.566 mol of H2 present. At equilibrium, there are __________ mol of Br2 present in the reaction vessel.

Student Response

Correct Answer

A. 0.000 B. 0.232 C. 0.440 D. 0.324 E. 0.566

11. chem10b 15.2-13 The equilibrium expression for Kp for the reaction below is __________. 2O3 (g)

3O2 (g)

Student Response

Correct Answer

A. B. C. [O2]3 / [O3]2 D. E.

12. chem10b 15.2-4 Which one of the following is true concerning the Haber process?

Student Response A. It is an industrial synthesis of sodium chloride that was discovered by Karl Haber. B. It is another way of stating LeChatelier's principle.

Correct Answer

C. It is a process for the synthesis of elemental chlorine. D. It is a process used for shifting equilibrium positions to the right for more economical chemical synthesis of a variety of substances. E. It is a process used for the synthesis of ammonia.

1.

chem10b 15.2-32 Consider the following reaction at equilibrium: 2NH3 (g)

N2 (g) + 3H2 (g) ΔH° = +92.4 kJ

Le Ch telier's principle predicts that adding N2 (g) to the system at equilibrium will result in __________.

Student Response

Correct Answer

A. an increase in the value of the equilibrium constant B. removal of all of the H2 (g) C. a decrease in the concentration of NH3 (g) D. a lower partial pressure of N2 E. a decrease in the concentration of H2 (g)

2.

chem10b 15.1-13 The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g)

PCl3 (g) + Cl2 (g)

A vessel is charged with PCl5, giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl3 is __________ atm.

Student Response A. 0.045 B. 0.033 C. 0.078

Correct Answer

D. 0.090 E. 0.123

3.

chem10b 15.4-5 Le Chatelier's principle states that if a system at equilibrium is disturbed, the equilibrium will shift to minimize the disturbance.

Student Response

4.

Value

Correct Answer

chem10b 15.5-4 At 900 K, the equilibrium constant (Kp) for the following reaction is 0.345. 2SO2 + O2 (g) → 2SO3 (g) At equilibrium, the partial pressure of SO2 is 35.0 atm and that of O2 is 15.9 atm. The partial pressure of SO3 is __________ atm.

Student Response

Correct Answer

A. 6.20 × 10-4 B. 82.0 C. 4.21 × 10-3 D. 40.2 E. 192

5.

chem10b 15.2-30 For the endothermic reaction CaCO3 (s)

CaO (s) + CO2 (g)

Le Ch telier's principle predicts that __________ will result in an increase in the number of moles of CO2.

Student Response

Correct Answer

A. removing some of the CaCO3 (s) B. increasing the temperature C. decreasing the temperature D. increasing the pressure E. adding more CaCO3 (s)

6.

chem10b 15.4-4 In an exothermic equilibrium reaction, increasing the reaction temperature favors the formation of reactants.

Student Response

Value

Correct Answer

False

0%

True

Score: 7.

0/1

chem10b 15.2-38 The effect of a catalyst on an equilibrium is to __________.

Student Response

Correct Answer

A. increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture B. increase the rate of the forward reaction only C. shift the equilibrium to the right D. slow the reverse reaction only E. increase the equilibrium constant so that products are favored

8.

chem10b 15.4-2 The effect of a catalyst on a chemical reaction is to react with product, effectively removing it and shifting the equilibrium to the right.

Student Response

Value

Correct Answer

9.

chem10b 15.1-1 The value of Keq for the equilibrium H2 (g) + I2 (g)

2 HI (g)

is 794 at 25 °C. What is the value of Keq for the equilibrium below? 1/2 H2 (g) + 1/2 I2 (g)

HI (g)

Student Response

Correct Answer

A. 28 B. 1588 C. 397 D. 0.035 E. 0.0013

10. chem10b 15.2-27 Nitrosyl bromide decomposes according to the following equation. 2NOBr (g)

2NO (g) + Br2 (g)

A sample of NOBr (0.64 mol) was placed in a 1.00-L flask containing no NO or Br2. At equilibrium the flask contained are in the flask at equilibrium?

of NOBr. How many moles of NO and Br2, respectively,

Student Response A. 0.46, 0.46 B. 0.18, 0.18 C. 0.18, 0.090 D. 0.18, 0.360 E. 0.46, 0.23

11. chem10b 15.2-14 The Keq for the equilibrium below is 7.52 × 10-2 at 480 °C.

Correct Answer

2Cl2 (g) + 2H2O (g)

4HCl (g) + O2 (g)

What is the value of Keq at this temperature for the following reaction?

Cl2 (g) + H2O (g)

2HCl (g) +

O2 (g)

Student Response

Correct Answer

A. 0.0752 B. 5.66 × 10-3 C. 0.0376 D. 0.274 E. 0.150

12. chem10b 15.2-23 The equilibrium-constant expression for the reaction Ti (s) + 2Cl2 (g)

TiCl4 (l)

is given by

Student Response

Correct Answer

A. [Cl2 (g)]-2 B. C. D. E. Score:

1/1

13. chem10b 15.1-9 At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103. 2NO (g)

N2 (g) + O2 (g)

A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is __________ atm.

Student Response

Correct Answer

A. 6.00 B. 18.1 C. 35.7 D. 294 E. 1.50 × 10-2 Score:

1/1

14. chem10b 15.1-11 In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g)

CO2 (g) + H2 (g)

In an experiment, 0.35 mol of CO and 0.40 mol of H2O were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.19 mol of CO remaining. Keq at the temperature of the experiment is __________.

Student Response

Correct Answer

A. 5.47 B. 1.78 C. 1.0 D. 0.75 E. 0.56

15. chem10b 15.2-12 Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide? N2O4 (g)

2NO2 (g)

Student Response

Correct Answer

A. [NO2][N2O4] B. C. [NO2]2[N2O4] D. [NO2]2 / [N2O4] E.

16. chem10b 15.2-5 Which one of the following will change the value of an equilibrium constant?

Student Response

Correct Answer

A. varying the initial concentrations of reactants B. changing temperature C. adding other substances that do not react with any of the species involved in the equilibrium D. varying the initial concentrations of products E. changing the volume of the reaction vessel

17. chem10b 15.1-4 Consider the following chemical reaction: H2 (g) + I2 (g)

2HI (g)

At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were and

respectively. The value of Keq for this reaction is __________.

Student Response A. 6.1 B. 111 C. 23 D. 9.0 × 10-3

Correct Answer

E. 61

18. chem10b 15.1-8 Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g)

2NO2 (g)

A 1.00-L flask is charged with .0400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is __________.

Student Response

Correct Answer

A. 2.2 × 10-4 B. 0.022 C. 0.22 D. 0.87 E. 13 Score:

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19. chem10b 15.5-5 The equilibrium constant (Kp) for the reaction below is 7.00 × 10-2 at 22 °C: NH4HS (s) → NH3 (g) + H2S (g) A sample of NH4HS is placed in an evacuated container and allowed to come to equilibrium. The partial pressure of NH3 is then increased by the addition of 0.590 atm of NH3. The partial pressure of H2S at equilibrium is now __________ atm.

Student Response A. 0.691 B. 0.119 C. 0.855 D. 0.265 E. 0.101

20. chem10b 15.2-35 Consider the following reaction at equilibrium:

Correct Answer

2CO2 (g) < -- > 2CO (g) + O2 (g) ΔH° = -514 kJ Le Chatelier's principle predicts that an increase in temperature will __________.

Student Response A. decrease the partial pressure of CO2 (g) B. decrease the value of the equilibrium constant C. increase the partial pressure of O2 (g) D. increase the value of the equilibrium constant E. increase the partial pressure of CO

Correct Answer